Non metals are likely to steal electron. They form anions.
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
This is an ionic bond.
Group 1 metals are very reactive because they have one electron in their outer shell, which they readily lose to achieve a stable electron configuration. Group 7 non-metals are very reactive because they are one electron short of a full outer shell, so they can easily accept an electron to achieve stability. This makes both group 1 metals and group 7 non-metals highly reactive in order to achieve a stable electron configuration.
Yes. The atom only bonds spontaneously if its to become more stable. So depending on the valence electrons, they have different forms of getting that stability. Let's see: Elements from the first and second group have 1 and 2 electrons of valence, respectively, so they tend to give them up. That's why they tend to bond with ionic bonds. They never steal electrons from others. Elements from the 17th group, are missing one electron to have their valence orbitals full, so again, they tend to steal electrons from those of group 1, forming stable ionic bonds. They can also give up some of their electrons, but more commonly they prefer to steal one. Elements like N and C, have their valence orbitals close to 50% filled, so they tend to prefer sharing electrons, that is, covalent bonds. Finally noble gases, have their valence orbitals filled with electrons, so they don't react with anything, and the only bonds they make, are weak Van der Waal bonds between themselves.
Ionic bond; ionic bonds occur when an element, mainly a metal, loses its electron ( to become positively charged) to an other element, mainly a nonmetal, ( to become negatively charged), to form an ionic compound. For example :- Na + Cl = NaCl
Both of the elements will have two different electronegativities. When there is a large difference between the two electronegativities, one element will "steal" one or more electrons from the other element. The energy required for this is ionization energy, and increases as an element takes more electrons from another. My answer: Elements are stabilized when they contain a "complete shell" or the noble gas configuration of electrons, which is usually eight electrons. Elements that have a number of electrons close to that of a noble gas, will lose or gain electrons easily. For example, elements in the column just to the left of the noble gases have one fewer electron than the noble gas next to it, and therefore they tend to gain one electron easily. Elements in the column on the far left of the periodic table have one more electron than the noble gas in each row, and they tend to lose one electron easily. Because the protons contribute the positive charge, and the electrons contribute the negative charge, an ion is formed when an element gains or loses one or more electrons.
Group 8 rarely forms ions since it has steal/lose more electrons to follow the octet rule (having eight valence electrons).
Oxygen is a really strong oxidizing agent, meaning it's really greedy with electrons. It really wants to become stable like the noble gases, who have completely filled electron shells. The only way to get electrons is to oxidize other elements and steal their electrons. That's why oxygen is so reactive.
In the short form: elements are striving to completely fill valence shells of electrons to reach a quantumly stable energy state. They react to take electrons away from elements willing to give up electrons or share outer shell electrons with elements they aren't strong enough to steal from.
Chlorine achieves stability by gaining one electron to complete its outer shell, forming a chloride ion with a negative charge. Chlorine can also share electrons with other elements to achieve stability through covalent bonds.
DCPIP acts as an electron acceptor of a Hill Reacton. In this way, it "steals" electrons.
The oxygen, nitrogen, and fluorine groups love to steal electrons from other elements, making them negatively charged ions, whereas most metals up to the carbon group like to give away electrons, making them positively charged ions. I hope that's what you were asking.
This is an ionic bond.
It is easier for this element, due to its electronegativity, to gain three electrons off other elements then to lose 5 of its own. Its like each elemnt has a strength. How strong an element is causes that element to be able to hold on to its own electrons and even steal electrons from other elements. Phosphorous is a relatively strong element. It can hold onto its original valence electrons quite well and won't let any of them go. It also can steal electrons from other elements that are weak enough to let their valence electrons go. Its like a tug of war. Phosphorous is strong so it holds its own side of rope (its own electrons) and can pull the other side of rope if the other element is weak.
Yes most likely there will be.
Francium and Flourine are the most reactive elements. Francium is at the bottom, Flourine is at the top. The trend isn't as simple as your question. Elements towards the top of the table "want" electrons more. This means they are less likely to give them up and more likely to "steal." In terms of reactivity, this means that the metals at the top are less reactive and the non-metals at the top are more reactive.
Group 1 metals are very reactive because they have one electron in their outer shell, which they readily lose to achieve a stable electron configuration. Group 7 non-metals are very reactive because they are one electron short of a full outer shell, so they can easily accept an electron to achieve stability. This makes both group 1 metals and group 7 non-metals highly reactive in order to achieve a stable electron configuration.